This question is about chemical equilibrium.
Nitrogen monoxide, NO\text{NO}NO, and oxygen, O2\text{O}_2O2, react to form nitrogen dioxide, NO2\text{NO}_2NO2, in the reversible reaction shown below:
2NO(g)+O2(g)⇌2NO2(g)ΔH=−114 kJ mol−1, ΔS=−146 J mol−1 K−1 2\text{NO}(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{NO}_2(\text{g}) \quad \Delta H = -114\text{ kJ mol}^{-1}, \; \Delta S = -146\text{ J mol}^{-1}\text{ K}^{-1} 2NO(g)+O2(g)⇌2NO2(g)ΔH=−114 kJ mol−1,ΔS=−146 J mol−1 K−1A dynamic equilibrium exists in a closed system. State one other feature of a dynamic equilibrium.
Show that the formation of NO2\text{NO}_2NO2 is feasible at 25∘C25^\circ\text{C}25∘C.
Determine the maximum temperature, in K\text{K}K, for feasibility. Give your answer to an appropriate number of significant figures.
A chemist mixes together 3.00 mol of NO(g)\text{NO}(\text{g})NO(g) and 2.00 mol of O2(g)\text{O}_2(\text{g})O2(g) in a container, and the mixture is allowed to reach equilibrium. At equilibrium, 75% of the NO(g)\text{NO}(\text{g})NO(g) has been converted to NO2(g)\text{NO}_2(\text{g})NO2(g), and the total pressure is 2.40 MPa.
Calculate KpK_pKp, in MPa−1\text{MPa}^{-1}MPa−1, for this reaction. Give your answer to 3 significant figures.
The chemist then repeats the experiment three times. In each experiment, the chemist makes one change but uses the same initial amounts of NO\text{NO}NO and O2\text{O}_2O2.
Complete the table to show the predicted effect of each change compared with the original experiment. Only use the words greater, smaller, or same.
| Change | KpK_pKp | Equilibrium amount of NO2(g)\text{NO}_2(\text{g})NO2(g) | Initial rate |
|---|---|---|---|
| Temperature increase | |||
| Pressure increase | |||
| Catalyst added |
